Two coordinatively linked supramolecular assemblies constructed from highly electron deficient porphyrins

Article abstract of DOI:10.1016/j.ica.2004.06.059

The synthesis of a pair of electron-deficient porphyrin building blocks and their resulting coordinatively linked supramolecular assemblies are described. The perfluorophenyl substituted porphyrins feature pendant pyridines which, upon reaction with Re(CO)₅Cl assemble into discrete dimers and tetramers, as dictated by the geometry of the porphyrin monomer. The resulting supramolecular complexes as well as their constituent porphyrins display several interesting and potentially useful properties owing to the electron-withdrawing nature of the perfluorophenyl funtionalities. Structural, spectroscopic, and electrochemical data indicate that the electron-deficient porphyrins remain planar, allowing for modulation of spectral and redox properties, as well as for enhancement of the affinity of the porphyrins for Lewis-basic ligands.

Full text of DOI:10.1016/j.ica.2004.06.059

Inorganica Chimica Acta 357 (2004) 4005–4014
www.elsevier.com/locate/ica
Two coordinatively linked supramolecular assemblies
constructed from highly electron deficient porphyrins
1
Kathryn E. Splan , Charlotte L. Stern, Joseph T. Hupp
*
Department of Chemistry, Northwestern University, 2145 Sheridan Road, Evanston, IL 60208, USA
Received 21 May 2004; accepted 26 June 2004
Available online 1 October 2004
Dedicated to Professor Tobin J. Marks on the occassion of his 60th birthday
Abstract
The synthesis of a pair of electron-deficient porphyrin building blocks and their resulting coordinatively linked supramolecular
assemblies are described. The perfluorophenyl substituted porphyrins feature pendant pyridines which, upon reaction with
Re(CO)5Cl assemble into discrete dimers and tetramers, as dictated by the geometry of the porphyrin monomer. The resulting
supramolecular complexes as well as their constituent porphyrins display several interesting and potentially useful properties owing
to the electron-withdrawing nature of the perfluorophenyl funtionalities. Structural, spectroscopic, and electrochemical data indi-
cate that the electron-deficient porphyrins remain planar, allowing for modulation of spectral and redox properties, as well as
for enhancement of the affinity of the porphyrins for Lewis-basic ligands.
ꢀ 2004 Elsevier B.V. All rights reserved.
Keywords: Porphyrins; Supramolecular complexes; Electrochemistry
1. Introduction
of dyads – variants of compound 1 – have been studied as
donor–acceptor complexes for energy transfer studies
[11]. Molecular square 2 can function as a component of
an artificial enzyme for epoxidation catalysis [12] and
forms thin films capable of size selective permeant trans-
port [13]. Closely related assemblies have been shown to
form free-standing polymeric membranes [14], while still
others are being used for photovoltaic applications [15].
Multiporphyrin arrays have proved to be an enormous
field of recent interest [1]. First and foremost, porphyrinsꢀ
close resemblance to natural light-harvesting chromoph-
ores have pushed them to the forefront of biomimetic
studies of Natureꢀs photosynthetic system and artificial
photosynthesis [2–5]. Since then, numerous applications
involving multiporphyrin systems have emerged. Porphy-
rins have been used in metallacyclic architectures as struc-
tural building blocks [6,7], sensor arrays [8], and
molecular electronics components [9]. Recent efforts in
our group have focused on the assembly of porphyrin
compounds based on rhenium–pyridine coordination
for a variety of applications [10–15]. For example, a series
CO
OC Re Cl
OC
H3CO
OCH3
N
N
N
N
Zn
N
N
N
N Zn
N
N
*
N
OC
OC
Corresponding author. Tel.: +847 491 3504; fax: +847 467 1425.
E-mail addresses: k-splan@chem.nwu.edu (K.E. Splan), j-hupp
N
OCH3
H3CO
Re Cl
CO
@northwestern.edu (J.T. Hupp).
1
Tel.: +847 467 4931.
1
0020-1693/$ - see front matter ꢀ 2004 Elsevier B.V. All rights reserved.
doi:10.1016/j.ica.2004.06.059

4006
K.E. Splan et al. / Inorganica Chimica Acta 357 (2004) 4005–4014
Recent advances in synthetic chemistry allow for func-
propionic acid. The mixture was deoxygenated by bub-
bling for 10 min with N2 and then refluxed for 2 h. The
solution volume was reduced by rotary evaporation
and methanol was added to precipitate the products,
yielding a mixture of six porphyrin isomers. The mixture
was loaded onto a silica column and the desired products
were eluted with 30:1 CHCl3:EtOH. The trans and cis iso-
mers eluted as the third and fourth band, respectively.
tionalization of porphyrin compounds in a remarkably
broad variety of ways [16]. Porphyrin building blocks
can be designed to assemble spontaneously in predicta-
ble, well defined, and organized ways, and can be further
functionalized to exhibit particular properties. Specifi-
cally, highly electron-deficient porphyrins containing
halogen functionalities have been the subject of much re-
search [17–21]. The electronegativity of the substituents
engenders unique structural and electronic changes that
can alter function. For example, polyhaloporphyrins
can display enhanced catalytic activity for oxidation
reactions [19], while fluorine substitution, in particular,
has also been found to play a modulating role in energy
and electron transfer rates through multiporphyrin ar-
rays [22,23]. Herein we describe a pair of electron-defi-
cient porphyrin building blocks (Scheme 1, 3 and 4)
and two resulting supramolecular assemblies (5 and 6).
The compounds display many of the interesting and
advantageous characteristics of other halogen-function-
alized porphyrins, and their implications are discussed
in the context of applications.
2.1.1.1. Characterization of 3a (cis isomer). Column
chromatography yielded only trace amounts (<1%);
therefore the product was collected and combined from
several reactions. 1H NMR (CDCl3, 400 MHz): 12.10 (s,
2H), 9.08 (d, 4H, J = 5.9 Hz), 8.86 (dd, 8H, J = 7.3 Hz),
8.17 (d, 4H, J = 5.9 Hz) ppm. Anal. Calc. for
C42H18N6F10: C, 63.31; H, 2.28; N, 10.55. Found: C,
63.31; H, 2.28; N, 10.37%. HRMS (FAB): 797.1511
(MH+, m/z calculated), 797.1516 (m/z observed). UV–
Vis (CH2Cl2): 414, 509, 540, 584, 647 nm. Fluorescence
(THF): 648, 710 nm.
2.1.1.2. Characterization of 4a (trans isomer). Yield: 2%.
1H NMR (CDCl3, 400 MHz): 12.04 (s, 2H), 9.07 (d, 4H,
J = 5.9 Hz), 8.87 (dd, 8H, J = 5.2 Hz), 8.17 (d, 4H,
J = 5.9 Hz) ppm. Anal. Calc. for C42H18N6F10: C,
63.31; H, 2.28; N, 10.55. Found: C, 63.05; H, 2.56; N,
10.46%. UV–Vis (CH2Cl2): 414, 510, 540, 586, 646 nm.
Fluorescence (THF): 649, 712 nm. LRMS (MALDI-
TOF): 797.2 (MH+, m/z calculated), 797.9 (m/z
observed).
R
R
N
N
N
N
N
N
Zn
Re(CO) Cl
3
N
Cl(CO) Re
3
N
R
R
R
R
R
R
N
Zn
N
N
N
N
Zn
N
N
N
R
R
2.1.2. [5,10-bis(pentafluorophenyl)-15,20-di(4-pyridyl)-
porphinato]zinc(II) (3b)
R
R
N
Zinc acetate (31.8 mg, 0.173 mmol) was dissolved in
MeOH (5 mL) and added to 3a (46.5 mg, 0.0584 mmol)
in CHCl3 (30 mL). The reaction stirred overnight in the
dark. The solvent was removed under reduced pressure
and the product recrsytallized from THF/hexanes. Upon
filtration, the purple solid was washed with 1:1
R
R
N
N
N
N
N
N
N
Cl(CO) Re
Re(CO) Cl
3
Zn
3
R
R
R= C H
4
9
2
1
H2O:MeOH (41.6 mg, 83% yield). H NMR (CDCl3/1
drop of py-d5): 8.88 (d, 4H), 8.84 (d, 2H), 8.78 (m, 6H),
8.05 (d, 4H) ppm. LRMS (MALDI-TOF): 859.1 (MH+,
m/z calculated), 859.2 (m/z observed). UV–Vis (CH2Cl2):
425, 556, 599 nm. Fluorescence (THF): 603, 656 nm.
2. Experimental section
2.1. Synthesis and characterization
The synthesis of porphyrin compounds 3–6 is out-
lined in Scheme 1 and is detailed below. The synthesis
of 3a and 4a is similar to a previous report [24]. All rea-
gents were used as received unless otherwise specified.
2.1.3. [5,15-bis(pentafluorophenyl)-10,20-di(4-pyridyl)-
porphinato]zinc(II) (4b)
The synthesis is as described above for 3b. Yield:
91%. 1H NMR (Acetone-d6/pyridine-d5, 400 MHz):
9.21 (d, 4H, J = 5.1 Hz), 9.01 (d, 4H, J = 5.9 Hz), 8.98
(d, 4H, J = 5.1 Hz), 8.23 (d, 4H, J = 5.9 Hz) ppm. Anal.
Calc. for C42H16N6F10 Æ H2O: C, 57.53; H, 2.07; N, 9.59.
Found: C, 57.36; H, 1.80; N, 9.52%. LRMS (MALDI-
TOF): 859.1 (MH+, m/z calculated), 859.6 (m/z ob-
served). UV–Vis (THF): 420, 552, 588 nm. Fluorescence
(THF): 604, 658 nm.
2.1.1. 5,10-bis(pentafluorophenyl)-15,20-di(4-pyridyl)
porphyrin (3a, cis isomer) and 5,15-bis(pentafluorophe-
nyl)-10,20-di(4-pyridyl)porphyrin (4a, trans isomer)
Pentafluorobenzaldehyde (4.909 g, 0.025 mol), freshly
distilled 4-pyridinecarboxaldehyde (2.678 g, 0.025 mol),
and pyrrole (3.357, 0.050 mol) were added to 150 mL of

K.E. Splan et al. / Inorganica Chimica Acta 357 (2004) 4005–4014
4007
N
F
F
F
O
H
N
HN
N
N
F
F
F
NH
F
F
F
F
F
F
F
F
+
F
3a
O
H
Acetic Acid, heat
+
F
N
F
F
+
N
F
F
N
HN
N
N
N
NH
F
F
F
F
F
4a
N
OC
CO
F
Re Cl
OC
F
F
F
N
N
F
F
F
F
F
F
N
N
N
N
F
2Re(CO)5Cl
THF, N2,
M
F
N
N
N
F
F
N M
N
N
N
N
M
N
F
F
F
F
F
F
F
F
F
60 hrs.
F
F
N
N
F
F
F
F
F
OC
OC
Re
Cl
CO
3a: M=H
2
3b: M=Zn
5a: M=H
2
5b: M=Zn
F
F
M
F
F
F
F
F
F
F
F
F
Cl
2Re(CO)5Cl
CO
Re
N
N
N
N
N
N
N
N
N
M
F
N
Re
CO
N
OC
OC
THF, N2,
60 hrs.
N
OC
CO
Cl
F
F
F
F
F
F
F
F
6a: M = H
4a: M=H
2
2
6b: M = Zn
4b: M=Zn
Scheme 1. Synthesis of porphyrin compounds 3–6.
2.1.4. Re(CO)3(l-(5,10-bis(pentafluorophenyl)-15,20-
di(4- pyridyl)porphyrin))Cl]2 (5a)
ppm. LRMS (FAB): 2204.6 (MH+ m/z, calculated),
2204.0 (m/z, observed). UV–Vis (THF): 422, 512, 588,
544, 644. Fluorescence (THF): 660, 718 nm.
3a (30.6 mg, 0.0384 mmol) and Re(CO)5Cl (14.3 mg,
0.0395 mmol) were refluxed under N2 in distilled THF
(25 mL) for 48 h. Upon cooling to room temperature,
hexanes were added to precipitate the product, which
was obtained as a purple solid (34.3 mg, 81%). 1H
NMR (CDCl3, 400 MHz):10.00 (br, 4H), 9.53 (br,
4H), 9.18 (d, 4H, J = 4.4 Hz), 9.05 (d, 4H, J = 4.4 Hz),
8.99 (s, 4H), 8.94 (s, 4H), 8.56 (br, 4H), 8.44 (br, 4H)
2.1.5. [Re(CO)3(l-([5,10-bis(pentafluorophenyl)-15,20-
di(4-pyridyl)porphinato]zinc(II))Cl]2 (5b)
Zinc acetate (10.6 mg, 0.0578 mmol) was dissolved in
MeOH (5 mL) and added to 5a (26.4 mg, 0.0120 mmol)
in CHCl3 (25 mL). The reaction mixture was stirred
overnight in the dark. The product precipitated upon

4008
K.E. Splan et al. / Inorganica Chimica Acta 357 (2004) 4005–4014
the addition of MeOH to yield 12.7 mg. 1H NMR (Ace-
tone-d6, 400 MHz): 9.78 (d, 4H, J = 5.1 Hz), 9.56 (d, 4H,
J = 5.9 Hz), 9.36 (s, 4H), 9.25 (d, 4H, J = 4.4 Hz), 9.21
(d, 4H, J = 5.1 Hz), 9.16 (s, 4H), 8.65 (d, 4H, J = 5.1
Hz), 8.58 (d, 4H, J = 5.1 Hz) ppm. UV–Vis (acetone):
422, 554, 596. Fluorescence (THF): 615, 662 nm.
pseudo-reference electrode. All potentials were measured
versus ferrocene and then adjusted to SCE based on
Ferr+/0 = 0.31 versus SCE in acetonitrile [25].
2.3. X-ray crystallography
X-ray quality crystals of 4a were grown from a
CHCl3 solution inside a capped NMR tube. Crystal data
are presented in Table 1. Data were collected using a
Bruker SMART detector and processed using SAINT-
NT from Bruker. The structure was solved by direct
methods and expanded using Fourier techniques. The
non-hydrogen atoms were refined anisotropically.
The central hydrogens were refined isotropically, and
the remaining hydrogen atoms were included in ideal-
ized positions. Neutral atom scattering factors [26],
anomalous dispersion effect values [27], and mass atten-
uation coefficients [27] were taken from literature values.
All calculations were performed using the Bruker SHEL-
XTL crystallographic software package [28].
2.1.6. [Re(CO)3(l-(5,15-bis(pentafluorophenyl)-10,20-
di(4-pyridyl)porphyrin))Cl]4 (6a)
4a (56.6 mg, 0.0711 mmol) and Re(CO)5Cl (26.1 mg,
0.0721 mmol) were refluxed under N2 in distilled THF
for 48 h. Upon cooling to room temperature, hexanes
were added to precipitate the product, which was ob-
tained as a purple solid (66.5 mg, 85%). 1H NMR (Ace-
tone-d6, 400 MHz): 9.60 (d, 16H, J = 6.6 Hz), 9.24 (br,
32H), 8.70 (d, 16H, J = 6.6 Hz) ppm. Anal. Calc. for
C
180H72N24F40O12Re4Cl4 Æ 4H2O: C, 47.45; H, 1.95; N,
7.38. Found: C, 47.43; H, 2.02; N, 7.18%. LRMS
(FAB): 4410.2 (MH+ m/z, calculated), 4410.8 (m/z, ob-
served). FT-IR (THF): mCO = 2023, 1921, 1886 cmꢀ1
.
UV–Vis (CH2Cl2): 418, 510, 586 nm. Fluorescence
(THF): 664, 714 nm.
2.4. Binding constant (Kb) determination
2.1.7. [Re(CO)3(l-([5,15-bis(pentafluorophenyl)-10,20-
di(4- pyridyl)porphinato]zinc(II))Cl]4 (6b)
Kb values for pyridyl ligands binding to porphyrin
squares 2 and 6b were determined by electronic absorp-
4b (56.4 mg, 0.0656 mmol) and Re(CO)5Cl (25.2 mg,
0.0697 mmol) were treated as above for 6a. Yield (68.9
1
mg, 90%). H NMR (Acetone-d6, s400 MHz): 9.56 (d,
Table 1
Crystallographic data for 4a
16H, J = 6.6 Hz), 9.17 (dd, 32H, J = 4.4), 8.64 (d, 16H,
J = 5.9 Hz) ppm. Anal. Calc. for C180H64N24F40O12R-
e4Cl4Zn4 Æ 8H2O: C, 44.98; H, 1.68, N, 6.99. Found: C,
44.23; H, 1.39; N, 6.92%. LRMS (FAB): 4663.7 (MH+
m/z, calculated), 4663.7 (m/z, observed). FT-IR (KBr):
Chemical formula
C42F10N6H18 Æ 2(CHCl3)
1035.38
red, plate
Formula weight (g/mol)
Crystal color, habit
Lattice parameters
˚
a (A)
6.7009(13)
10.305(2)
15.330(3)
86.739(3)
85.306(3)
77.309(3)
153 (2)
CO = 2025, 1927, 1887 cmꢀ1. UV–Vis (acetone) kmax (e)
˚
b (A)
m
˚
c (A)
[nm (cmꢀ1 Mꢀ1)] 422 (1,000,000), 552 (79,000). Fluores-
cence (CH2Cl2): 614, 650 nm.
a (ꢁ)
b (ꢁ)
c (ꢁ)
Temperature (K)
2.2. Instrumentation and methods
˚
Wavelength (A)
0.71073
ꢀ
Space group
Crystal dimensions (mm)
Crystal system
P1
Elemental analyses were performed by Atlantic
Microlabs, Inc. (Norcross, GA). Mass spectrometry data
were obtained from the University of Illinois, Urbana-
0.38 · 0.16 · 0.05
triclinic
1028.4(3)
2
3
˚
Volume (A )
1
Champaign Mass Spectrometry Center. H NMR spec-
Z value
Dcalc (g/cm3)
1.672
0.7107
tra were collected on a Mercury 400 MHz spectrometer.
Electronic absorption spectra were recorded on a Hewlett
Packard HP8452A diode array UV–Vis spectrophotom-
eter or a Varian Cary 5000 UV–Vis–NIR spectropho-
tometer. Steady-state fluorescence measurements were
performed on a Jobin Yvon-SPEX Fluorolog-3 spectro-
fluorimeter. Electrochemical data were obtained using a
CH Instruments potentiostat and plotted using CHI ver-
sion 1202 software. Unless otherwise stated all measure-
ments were conducted in dimethyl formamide with 0.1 M
tetrabutylammonium hexafluorophosphate (TBAPF6) as
supporting electrolyte using a glassy carbon working
electrode, platinum counter electrode, and Ag/AgCl
˚
Radiation MoKa k (A)
Graphite monochromated
Absorption coefficient (mmꢀ1
Maximum and minimum
transmission factors
Absorption correction
F (000)
)
0.507
0.9778 and 0.8844
integration
518
2h Range
1.33–28.28ꢁ
9474
Reflections collected
Unique reflections
Refinement method
Final R indices
4760
full-matrix least-squares on F2
0.0444 (R1), 0.1099 (wR2)
0.0644 (R1), 0.1290 (wR2)
1.54
R indices (all data)
Goodness-of-fit indicator

K.E. Splan et al. / Inorganica Chimica Acta 357 (2004) 4005–4014
4009
tion titration. For example, 10 lL aliquots of a 3.1 mM
solution of 4-phenylpyridine in CH2Cl2 were added to 2
mL of a 2.0 lM solution of 6b in CHCl3 and the absorb-
ance at 422 nm was recorded after each addition. The
data were fit to the following equation to obtain a value
for Kb:
structural identity of the isolated isomers ambiguous.
(Cleaner NMR-based assignments were reported, how-
ever, in [24] based on higher resolution measurements.)
Fortunately, crystals of an isolated porphyrin com-
pound, with mass spectral data corresponding to an iso-
mer, were suitable for X-ray diffraction studies, and the
compound was revealed to be the trans isomer. The re-
fined crystal structure of 4a is presented in Fig. 1 and se-
lected bond lengths and angles are reported in Table 2.
The structure reveals only a slightly ruffled porphyrin
macrocycle, with the largest deviations being only 0.19
ðKꢁb½guestꢂꢁDIÞ
Iobs
¼
þ Io;
ð1Þ
ðI þ ðKꢁb½guestꢂÞÞ
where I obs is the absorbance observed after each aliquot
addition, DI is the overall change in absorbance, and Io
is the initial absorbance. Eq. (1) assumes that for hosts
capable of binding multiple guests, allosteric effects
can be neglected. In applying the equation, account
was taken of the decrease in concentration of the guest
by guest:host association. For experiments in which
CH2Cl2 was used as the solvent, the concentration of
6b was estimated from the extinction coefficient meas-
ured in acetone, due to the low solubility of 6b in
CH2Cl2.
˚
A from the plane of the porphyrin ring (as defined by
the four central nitrogen atoms). The pyridyl and per-
fluorphenyl groups are oriented at 68.3ꢁ and 73.3ꢁ,
respectively, with regard to the plane of the porphyrin.
In short, the structure is quite similar to that of free-base
tetraphenyl porphyrin [31], implying that the electron-
withdrawing nature of the substituents has little, if
any, geometric structural impact. In contrast, porphy-
rins bearing perfluorinated alkyl chains at the meso
and beta positions are characterized by strongly dis-
torted and ruffled macrocycle structures, owing to unu-
3. Results and discussion
sual
hydrogen
bonding
interactions
between
fluorocarbon fluorine atoms and porphyrin NH protons
[21,32]. However, in the case of 4a and other perfluoro-
phenyl porphyrin compounds, the fluorine atoms of the
phenyl groups lie above and below the plane of the por-
phyrin, thereby precluding any intermolecular interac-
tions that might lead to ruffling [18]. Upon structural
assignment of the isomers, the order of elution was
established to be 4a followed by 3a. Surprisingly, the
trans isomer 4a was obtained in higher yield than the
cis isomer 3a, in contrast to the commonly observed
threefold preference for cis isomer formation under the
given experimental conditions [30].
3.1. Synthesis and characterization
Free base porphyrins 3 and 4 were prepared via Ad-
ler–Longo conditions [29]. It should be noted that the
compounds are briefly described in an earlier report by
Aviezer and coworkers were they are used as synthetic
intermediates [24]. Under these conditions, isomeric
compounds in which the pyridyl groups are either cis
(in the 5,10-positions) or trans (in the 5,15-positions)
to each other are formed and can be isolated via careful
column chromatography. Fluorinated porphyrin dimers
5 and tetramers 6 were synthesized as previously re-
ported for related compounds 1 [11] and 2 [10]. Briefly,
stoichiometric amounts of either cis or trans dipyridyl
porphyrins and Re(CO)5Cl were refluxed for two days
in THF to yield porphyrin dimers and squares, respec-
tively. The presence of electron withdrawing fluorine
groups on the monomers appeared not to greatly lower
the Lewis-basicity of the pyridyl groups, as longer reac-
tion times were not needed for the synthesis of 5 and 6
relative to 1 and 2. Note also that several geometrical
isomers are formed in the synthesis of 5 and 6 with re-
spect to the chloro-ligand orientation; no attempts were
made to separate these isomers.
3.3. Electronic structure effects
Although the perfluorophenyl groups have little effect
upon core porphyrin geometries, their presence results
in interesting electronic structural effects, which are best
described by the four-orbital model for porphyrin
ground and excited states [33,34]. The porphyrin lowest
unoccupied molecular orbital (LUMO) consists of two
degenerate orbitals of eg symmetry, while the two high-
est occupied molecular orbitals (HOMOs) are assigned
to a1u and a2u symmetry and are typically close in en-
1
1
ergy. When E(a1u, eg) and E(a2u, eg) are degenerate
the two transitions partially cancel, resulting in a very
low intensity band for the Q(0,0) transition, but leaving
the higher energy Q(1,0) transition unaffected. As the
degeneracy of the HOMOs is lifted the Q(0,0) band
gains intensity; therefore the ratio of Q(1,0) intensity
to Q(0,0) intensity reflects the energy difference between
the a1u and a2u orbitals. The Q-band region of the elec-
tronic absorption spectrum for compound 3b is shown
3.2. X-ray crystallography studies
Although the isomers have the same mass, elemental
composition, and photophysical properties, the identity
of the compounds can usually be determined by charac-
teristic NMR spectra [30]. However, 3 and 4 give extre-
mely similar NMR spectra (not shown) leaving the

4010
K.E. Splan et al. / Inorganica Chimica Acta 357 (2004) 4005–4014
Fig. 1. ORTEP representation of 4a showing both the front view (top) and side view (bottom) of the structure.
Table 2
0.4
Selected bond lengths and angles
˚
Bond lengths (A)
Bond angles (ꢁ)
0.3
0.2
0.1
0.0
N(2)–H(1)
N(2)–C(6)
C(6)–C(7)
C(7)–C(8)
C(5)–C(6)
C(10)–C(17)
C(5)–C(11)
0.81 (3)
C(6)–N(2)–H(1)
C(6)–N(2)–C(9)
N(2)–C(6)–C(5)
N(2)–C(6)–C(7)
C(8)–C(7)–C(6)
C(6)–C(5)–C(4)
C(5)–C(6)–C(7)
126 (2)
1.371(3)
1.434 (3)
1.364 (3)
1.397 (3)
1.494 (3)
1.494 (3)
109.8 (2)
126.3 (2)
107.0 (2)
108.0 (2)
126.6 (2)
126.6 (2)
in Fig. 2, along with the spectrum for the zinc complex
of 5,10,15,20-tetraphenyl porphyrin (ZnTPP). Relative
to ZnTPP, the intensity ratio of the Q(1,0) and Q(0,0)
transitions is large, with the Q(0,0) band appearing quite
weak. This implies that the a2u and a1u orbitals are clo-
ser in energy in compound 3b than in ZnTPP.
500
520
540
560
580
600
620
640
Wavelength (nm)
Fig. 2. Q-band region of the electronic absorption spectrum for
compound 3b (—) and ZnTPP (---) recorded in THF.
The different nodal pattern for the a1u and a2uorbitals
revealed by electron density maps (Scheme 2, top) ren-
ders the orbital energies sensitive to substitution at the
meso positions. Since the perfluorophenyl groups are
strongly electron withdrawing, they should act to lower
the orbital energy of a2u relative to a1u. Based on the
above discussion, the a1u and a2u orbitals are expected
to be close in energy, and the relative orbital order is
dependent on the porphyrin substituents. For example,
electronic structure calculations show that the HOMO
of the tetraphenylporphryin zinc complex (ZnTPP) is

K.E. Splan et al. / Inorganica Chimica Acta 357 (2004) 4005–4014
4011
is summarized in Table 3. Consistent with previous re-
ports [18,20], the electron withdrawing nature of the per-
fluorophenyl groups causes a positive shift in the
oxidation and reduction potentials for both the porphyrin
monomers and dimers, relative to the methoxyphenyl
substituted compounds. While the reduction potentials
are shifted positive by an average of 175 mV, the effect
is more dramatic for the oxidation potentials; shifts of
nearly 400 and 300 mV are observed for the porphyrin
and the dimer, respectively. (We have assumed that the
shifts in oxidation potential for these chemically irrevers-
ible processes reasonably approximate the thermodynam-
ically significant shifts that would be obtained if the
reactions were reversible.) Owing to the symmetry, and
therefore, the nodal patterns of the a1u and a2u and eg
orbitals, it follows that the potentials for oxidation com-
pounds should be more susceptible to modulation via
electron withdrawing (or donating) functionalities than
those for reduction.
While electron-withdrawing groups are capable of sta-
bilizing the porphyrin HOMO (as reflected in the oxida-
tion potential), the extent of the affect is dependent on
the structural characteristics of the compound as well.
Non-planar distortions of the porphyrin ring previously
Scheme 2. (a) Electron density maps of molecular orbitals a1u and a2u
.
(b) Molecular orbital diagram describing the effects of perfluorophenyl
substitution at the meso positions. The energy spacing between the
HOMO and HOMO-1 is larger for ZnTPP than for 3a and the orbital
symmetry is reversed.
2e-6
0
of a2usymmetry [17], while the HOMO of 3b is of a1u
symmetry [35]. Thus, as the phenyl groups of ZnTPP
are replaced with perfluorophenyl groups, the a2u orbital
is lowered in energy such that the orbital order is re-
versed (Scheme 2, bottom). The ability to manipulate
the orbital ordering, and thus, the electron density pat-
tern, is an important tool in the rational design of
molecular architectures that exploit electronic communi-
cation. Lindsey and co-workers have successfully modu-
lated singlet energy transfer (EnT) within covalently
linked porphyrin dyads via perfluorophenyl substitution
at the meso positions [22]. Briefly, energy transfer was
either: (a) kinetically inhibited by locating HOMO
nodes (a1u orbitals) at the meso carbon atoms used for
covalent linkage of the donor and acceptor porphyrins,
or (b) kinetically enhanced by locating nodes elsewhere
(a2u orbitals). Similar effects might be observed in asym-
metric (i.e. partially metallated) analogues of 1 and 5 in
which the difference in metallation creates a porphyrin/
porphyrin excited-state energy difference.
-2e-6
-4e-6
-6e-6
-8e-6
1.6
1.4
1.2
1.0
0.8
0.6
0.4
0.2
0.0
Potential vs.SCE
4e-6
3e-6
2e-6
1e-6
0
3.4. Electrochemistry
-1e-6
The redox potentials of several of the fluorinated com-
pounds were measured by cyclic voltammetry and
compared to those of 4-methoxyphenyl-substituted cis-
DPyP and 1. The cyclic voltammograms of 3a and cis-
DPyP are shown in Fig. 3 and the electrochemical data
-2e-6
0.0 -0.2 -0.4 -0.6 -0.8 -1.0 -1.2 -1.4 -1.6 -1.8 -2.0
Potential vs. SCE
Fig. 3. Cyclic voltamograms in the oxidation (top) and reduction
(bottom) regions for 3a (ꢃ ꢃ ꢃ) and cis-DPyP (—).

4012
K.E. Splan et al. / Inorganica Chimica Acta 357 (2004) 4005–4014
Table 3
Electrochemistry data for selected compounds
1.0
0.5
2.0
1.5
1.0
0.5
0.0
Compound
Eox1(V)a
Ered1(V)a
Ered2(V)a
0.0
cis-DPyP
0.94
1.33
1.02
1.31
ꢀ1.10
ꢀ0.91
ꢀ1.01
ꢀ0.85
ꢀ1.54
ꢀ1.38
n.a.b
n.a.b
3a
1
-0.5
-1.0
5a
a
V versus SCE. All data were taken in 0.1 M TBAPF6 DMF
electrolyte versus pseudo Ag/Agcl. Ferrocene was used as an internal
standard to convert all values to SCE reference.
0.0
4.0e-5
8.0e-5
1.2e-4
[4-phenylpyridine]
b
The second reduction potential for the porphyrin dimer com-
pounds was ambiguous owing to the Re(I/O) couple at similar pot-
entials and is not reported.
350
400
450
500
550
600
650
Wavelength (nm)
observed with bulky fluorinated substituents are known
to raise the HOMO energy, partially counteracting the
gains made by electron-withdrawing substitution [21,32].
For example, the oxidation potential of 2-bromo-
H2TPP is shifted 80 mV positive with respect to H2TPP
[36], while the addition of seven more bromine atoms fur-
ther shifts the potential by only 220 mV [37]. The absence
of planar distortions for 4a allows for the substantial 400
mV shift in apparent oxidation potential upon addition of
only two perfluorophenyl groups and reiterates the virtues
of structural invariance when seeking to modulate the
electronic properties via ligand substitution.
Fig. 4. Electronic absorption spectra of 6b upon the addition of 4-
phenylpyridine. Complete ligation by 6b is indicated by an 8 nm red-
shift in the Soret region. (Inset): Binding curve for the titration data.
Kb = (1.35 0.09) · 105 Mꢀ1
.
hanced Lewis base affinity of 6b is potentially useful.
For example, encapsulation by 2 of di-pyridyl manga-
nese porphyrin (MnDPyP), a known epoxidation cata-
lyst, results in a 10–100-fold enhancement in catalyst
lifetime (total turnover number), and further modifica-
tion of the catalyst to increase its affinity for 2 results
in even larger turn-over numbers [12]. Replacement of
2 with 6b would be expected to further enhance catalyst
performance.
Many construction schemes for multiporphyrin arrays
rely on axial coordination [38–40], and such interactions
can be enhanced to yield more robust structures by sim-
ple modification with electron-withdrawing functionali-
ties. For example, upon treatment with one equivalent
of a trans ditopic N-donor ligand, porphyrin dimers
and oligomers similar to 1 and 5b form discrete sandwich
complexes in which the di-functional ligands form
bridges between the porphyrin compounds [40,41]. The
sandwich structure is thermodynamically favored over
oligomeric structures or single point binding owing to a
cooperative effect upon zinc center ligation. As a result,
sandwich formation occurs on an all-or-nothing basis,
as no intermediates are observed in the UV–Vis spectra
[41].
3.5. Binding studies of porphyrin dimers and squares
Molecular squares 2 and 6b are capable of binding a
wide variety of pyridine-based guests via Zn axial liga-
tion. Upon exposure to excess 4-phenylpyridine in chlo-
roform as solvent the Soret band of 6b at 422 nm
experiences an 8 nm red-shift, indicative of zinc ligation
(Fig. 4). Only four, rather than eight, equivalents of
guest are expected to bind because of the preference of
Zn (II) for fivefold coordination. The binding constant
for 4-phenylpyridine in 6b was measured via an elec-
tronic absorption titration (Fig. 4, inset). The data were
fit to Eq. (1) to yield a Kb value of (1.35 0.09) · 105
M
ꢀ1, nearly an order of magnitude higher than for 2
as host (Kb = 1.5 · 104 ꢀ1). The perfluorophenyl
M
groups significantly increase the Lewis acidity of the zinc
center, resulting in an increased affinity for Lewis basic
pyridyl compounds. Also, the porphyrin-square/pyr-
idyl-ligand interaction is highly dependent on solvent,
as the binding constant for 4-phenylpyridine in 6b is
found to be over an order of magnitude smaller in ace-
tone, a moderately basic solvent that can compete to
some degree for the zinc binding site. Thus, in order
to fully exploit the enhanced binding capabilities of
complexes such as 6b it is important that they be suffi-
ciently soluble in non-coordinating solvents such as
CH2Cl2 and CHCl3.
N
N
N
N
7
Axial zinc binding is a helpful tool in the use of por-
phyrin compounds as functional assemblies, and the en-
= 5b

K.E. Splan et al. / Inorganica Chimica Acta 357 (2004) 4005–4014
4013
Consistent with these reports, treatment of 5b with
stoichiometric amounts of 4,40-bipyridine at micromolar
concentrations results in spectral shifts indicative of zinc
ligation. By analogy to the reports mentioned above for
closely related compounds, association is believed to
yield the sandwich structure 7. Based on this assump-
tion, the titration data can be analyzed using the fitting
program SPECFIT/32TM to yield a formation constant
rins display interesting and potentially usefully altered
properties owing to the electron-withdrawing nature of
the perfluorophenyl functionalities. Despite the presence
of fluorine atoms, which increase the likelihood of inter-
molecular hydrogen bonding, the geometrical structures
of the porphyrins remain relatively unperturbed. There-
fore, it is possible for the electron-deficient substituents
to alter the HOMO orbital energies significantly, as evi-
denced by substantial positive shifts in porphyrin oxida-
tion potentials. The addition of perfluorophenyl groups
enhances the affinity of porphyrin square 6b for pyri-
dine-based ligands owing to the increased Lewis acidity
of the zinc center. This enhanced affinity can be
exploited to form other supramolecular complexes such
as 7. Taken together, 3–7 illustrate in a straightforward
way how modification of porphyrin compounds with
electron-deficient substituents can impart or alter spe-
cific properties. Such modulation should prove useful
in applications that require careful control over struc-
tural, electronic, and supramolecular properties.
(Kf) of (2.8 1.2) · 1018
M
ꢀ3, where Kf is defined as:
½5b2ðbipyÞ ꢂ
2
Kf ¼
:
ð2Þ
2
2
½5bꢂ ½bipyꢂ
This value is consistent with those reported for simi-
lar porphyrin dimers [41]. In contrast, addition of 4-phe-
nylpyridine to micromolar amounts of 5b is best
modeled by 1:1 porphyrin:ligand complex formation,
assuming that the porphyrin centers in each dimer be-
have independent of one another, as previously ob-
served [41]. In this case a Kf value of (1.8 0.2) · 105
Mꢀ1 is observed. It is difficult to compare the strengths
of the two different interactions (sandwich formation
versus single point binding) because the dimensions of
Kf vary with different complexing species. A better point
of comparison is to calculate the concentration, c50, at
which each complex is 50% dissociated. For complex
7, c50 is calculated according to Eq. (3) [41]:
Acknowledgements
We thank the Basic Energy Sciences Program, Office
of Science, US Department of Energy (Grant No. DE-
FG02-87ER13808) and the Dow Foundation (graduate
fellowship to K.E.S.) for financial support of our
research.
1
c50
¼
:
ð3Þ
1=3
ð16Kf Þ
For simple 1:1 complex formation with 4-phenylpyri-
dine c50 is defined as 1/Kf. Values of 2.8 · 10ꢀ7 and
5.6 · 10ꢀ6 M are observed for 7 and 5b: 4-phenylpyri-
dine, respectively. This order of magnitude difference re-
flects the cooperative nature of the formation of 7 versus
single point binding. Note also, the enhanced basicity of
4-phenylpyridine (pKa = 5.55) versus 4,40-bipyridine
(pKa = 4.82) [42]. Comparisons with ligands having
more precisely matched pKa values should yield some-
what larger differences in c50 values. Finally, a similar
titration performed with 4,40-bipyridine and 1, again
presumably leading to sandwich structure formation,
yields Kf equal to (3.1 0.5) · 1016 Mꢀ3 and c50 equal
to 1.3 · 10ꢀ6 M. The enhanced Lewis-acidity of 5b rela-
tive to 1 clearly allows for the formation of a somewhat
more robust supramolecular architecture.
References
[1] C.M. Drain, J.T. Hupp, K.S. Suslick, M.R. Wasielewski, J.
Porph. Phthalocyanines 6 (2002) 243.
[2] D. Gust, T.A. Moore, Science 244 (1989) 35.
[3] H. Kurreck, M. Huber, Angew. Chem. Int. Ed. 34 (1995) 849.
[4] D. Kuciauskas, P.A. Liddell, S. Lin, T.E. Johnson, S.J. Weghorn,
J.S. Lindsey, A.L. Moore, T.A. Moore, D. Gust, J. Am. Chem.
Soc. 121 (1999) 8604.
[5] D. Gust, T.A. Moore, A.L. Moore, Acc. Chem. Res. 34 (2001) 40.
[6] J. Fan, J.A. Whiteford, B. Olenyuk, M.D. Levin, P.J. Stang, E.B.
Fleischer, J. Am. Chem. Soc. 121 (1999) 2741.
[7] E. Iengo, B. Milani, E. Zangrando, S. Germia, E. Alessio, Angew.
Chem. Int. Ed. 39 (2000) 1096.
[8] N.A. Rakow, K.S. Suslick, Nature 406 (2000) 710.
[9] A.S. Lukas, P.J. Bushard, M.R. Wasielewski, J. Am. Chem. Soc.
123 (2001) 2440.
[10] R.V. Slone, J.T. Hupp, Inorg. Chem. 36 (1997) 5422.
[11] K.E. Splan, M.H. Keefe, A.M. Massari, K.A. Walters, J.T.
Hupp, Inorg. Chem. 41 (2002) 619.
4. Conclusions
[12] M.L. Merlau, W.J. Grande, S.T. Nguyen, J.T. Hupp, J. Mol.
Catal. A: Chem. 156 (2000) 79.
In summary, cis and trans isomers of di-pyridyl por-
phyrin compounds featuring perfluorophenyl groups at
two of the four meso positions have been prepared and
reacted with Re(CO)5Cl to form dimeric and tetrameric
(square) porphyrin assemblies, respectively. The supra-
molecular assemblies as well as their constituent porphy-
[13] S. Belanger, J.T. Hupp, Angew. Chem. Int. Ed. 38 (1999) 2222.
[14] M.H. Keefe, J.L. OꢀDonnell, R.C. Bailey, S.T. Nguyen, J.T.
Hupp, Adv. Mater. 15 (2003) 1936.
[15] K.E. Splan, A.M. Massari, J.T. Hupp, J. Phys. Chem. B 108
(2004) 4111.
[16] S. Shanmugathasan, C. Edwards, R.W. Boyle, Tetrahedron 56
(2000) 1025.

4014
K.E. Splan et al. / Inorganica Chimica Acta 357 (2004) 4005–4014
[17] P.J. Spellane, M. Gouterman, A. Antipas, S. Kim, Y.C. Liu,
Inorg. Chem. 19 (1980) 386.
[28] SMART Version 5.054 Data Collection and SAINT-Plus Version
6.02A Data Processing Software for the SMART System; Bruker
Analytical X-ray Instruments: Madison, WI, 2000.
[29] A.D. Adler, F.R. Longo, J.D. Finarelli, J. Goldmacher, J. Assour,
L. Korsakoff, J. Org. Chem. 32 (1967) 476.
[18] E.K. Woller, S.G. DiMagno, J. Org. Chem. 62 (1997) 1588.
[19] D. Dolphin, T.G. Traylor, L.Y. Xie, Acc. Chem. Res. 30 (1997)
251.
[20] K.T. Moore, J.T. Fletcher, M.J. Therien, J. Am. Chem. Soc. 121
(1999) 5196.
[30] G.G. Meng, B.R. James, K.A. Skov, Can. J. Chem. 72 (1994)
1894.
[21] V.V. Smirnov, E.K. Woller, D. Tatman, S.G. DiMagno, Inorg.
Chem. 40 (2000) 2614.
[31] S.J. Silvers, A. Tulinsky, J. Am. Chem. Soc. 89 (1967) 3331.
[32] S.G. DiMagno, R.A. Williams, J. Org. Chem. 59 (1994) 6943.
[33] M. Gouterman, J. Chem. Phys. 30 (1959) 1139.
[34] M. Gouterman, in: D. Dolphin (Ed.), The Porphyrins, vol. III,
Academic Press, New York, 1979, p. 1.
[22] J.P. Strachan, S. Gentemann, J. Seth, W.A. Kalsbeck, J.S.
Lindsey, D. Holten, D.F. Bocian, J. Am. Chem. Soc. 119 (1997)
11191.
[23] A. Willert, S. Bachilo, U. Rempel, A. Shulga, E. Zenkevich, C.v.
Borczyskoski, J. Photochem. Photobiol. A: Chemistry 126 (1999)
99.
[35] M.H. Keefe, Ph.D. thesis, Department of Chemistry, Northwest-
ern University, 2001.
[36] A. Giraudeau, H.J. Callot, M. Gross, Inorg. Chem. 18 (1979) 201.
[37] P. Bhyrappa, V. Krishnan, Inorg. Chem. 30 (1991).
[38] R.A. Haycock, A. Yartsev, U. Michelsen, V. Sundstrom, C.A.
Hunter, Angew. Chem. Int. Ed. 39 (2000) 3616.
[24] D. Aviezer, S. Cotton, M. David, A. Segev, N. Khaselev, N.
Gahili, Z. Gross, A. Yayon, Cancer Res. 60 (2000) 2973.
[25] A.J. Bard, L.R. Faulkner, Electrochemical Methods: Fundamen-
tals and Applications, second ed., John Wiley & Sons Inc., New
York, 2001.
[39] K. Ogawa, Y. Kobuke, Angew. Chem. Int. Ed. 39 (2000) 4070.
[40] E. Iengo, E. Zangrando, R. Minatel, E. Alessio, J. Am. Chem.
Soc. 124 (2002) 1003.
[26] D.T. Cromer, J.T. WaberInternational Tables for X-ray Crystal-
lography, vol. IV, The Kynoch Press, Birmingham, England,
1974.
[41] P.N. Taylor, H.L. Anderson, J. Am. Chem. Soc. 121 (1999)
11538.
[27] D.C. Creagh, J.H. HubbellInternational Tables for Crystallogra-
phy, vol. C, Kluwer Academic Publishers, Boston, 1992.
[42] S. Belanger, M.H. Keefe, J.L. Welch, J.T. Hupp, Coord. Chem.
Rev. 190–192 (1999) 29.